Formula: CuO
Atomic weights:
Cu- 63.5 g
O- 16.0 g
Add together (molecular mass): 79.5 g
Take the weight of copper and divide it by the total molecular mass.
63.5 / 79.5 = 79.2% Cu
There is 79.2% of copper in copper II oxide
Since you know how much Copper weighs and how much Chloride weighs...
Copper=63.55
Chloride=35.45
So, you add 63.55 (Cu) to 35.45 (Cl) and you get 99.00 (<-- you want 4 sig. fig.'s since you have 4 sig. fig.'s for Cu and Cl.)
From here, you get the mass of Cu and u divide by the total mass of Cu(II)Cl.
63.55/99.00=.64191919192 (<-- since we are doing % composition, we multiply by 100)
. 64191919192 x 100 = 64.19% (<-- four sig. fig.'s again DON'T FORGET... VERY CRUCIAL)
Next, we fine Chloride...
35.45/99.00=.358080808080 (<-- since we are doing % composition, we multiply by 100)
.358080808080 x 100 = 35.80% (<-- four sig. fig.'s again DON'T FORGET... VERY CRUCIAL)
In the end, we get Copper is 64.19% and Chloride is 35.80%
P.S. in case you want to check, add the two percentage's up... they should equal 100 or at least something VERY close...
In this case, we get 99.99% (<-- prob. rounding error but pretty close)
Cu = 63.5 g/moleO = 16 g/mole
Copper(II) oxide = CuO = 63.5 + 16 = 79.5 g/mole
%Cu = 63.5/79.5 (x100) = 79.9%
NOTE: If you meant copper(I) oxide, it would be Cu2O and the calculation can be done the same way, but the % Cu will be greater (88.8%)
Copper(I) sulfide - Cu2S - has 79,75 % copper.
Copper I Chloride is CuCl and Copper II Chloride CuCl2
Hydrated copper(II) Chloride - CuCl2.5H2O
+2 oxidation state
CuCl2 + 2AgNO3 -------> Cu(NO3)2 + 2AgCl for Copper (II) Chloride CuCl + AgNO3 --------> CuNO3 + AgCl for Copper (I) Chloride
Copper (III) chloride. Note that this is theoretical compound copper does have a +3 oxidation stae in some complexes but does not from compounds such as CuCl3. The only halides known are +1 oxdtn state:- CuCl, CuBr, CuI +2 oxdtn state : CuF2, CuCl2, CuBr2
Copper I Chloride is CuCl and Copper II Chloride CuCl2
Hydrated copper(II) Chloride - CuCl2.5H2O
Copper(II) chloride and Silver metalCu + 2 AgCl ----> CuCl2 + 2 Ag
Copper (II) Chloride is CuCl2
+2 oxidation state
CuCl2 + 2AgNO3 -------> Cu(NO3)2 + 2AgCl for Copper (II) Chloride CuCl + AgNO3 --------> CuNO3 + AgCl for Copper (I) Chloride
Chemical Formula of Copper Chloride is CuCl2
CuCl2+NaOH= Cu(OH)2+Na2Cl
Copper (III) chloride. Note that this is theoretical compound copper does have a +3 oxidation stae in some complexes but does not from compounds such as CuCl3. The only halides known are +1 oxdtn state:- CuCl, CuBr, CuI +2 oxdtn state : CuF2, CuCl2, CuBr2
Some Cu(HCO3)2 or CuCO3 precipitation might occur.
There are two different copper chloride compounds, due to the two possible 'oxidation state numbers' (+1 and +2):CuCl cuprous chloride, Cu(I) chloride, mono-valent Copper chlorideCuCl2 cupric chloride, Cu(II) chloride, bi-valent Copper chloride
Copper Chloride